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25.4 g of I2 and 14.2 g of Cl2 are made to react completely to yield a mixture of ICl and ICl3 . Calculate mole of ICl and ICl3 formed.
1. Consider a process involving 1 mole of an ideal gas that takes place by the following pathway, at a constant temperature of 25oC: P1 = 2.5 atm → P2 = 0.25 atm → P3 = 2.5 atm Both steps occur irreversibly.
a sample of Ringer's solution contains the following concentractions (mEq/L) of cations: Na 147, K 4 and Ca2 4. If CI- is the only anion in the solution
a 11.7 ml sample of a hcl solution has a ph of 2.000. what volume of water must be added to change the ph to
an aqueous solution containing 34.1 g of an unknown molecular nonelectrolyte compound in 141.3 g of water was found to
Calculate the work done by the gas if it expands against a constant pressure of 5 atm. -Answer is -1.14x10^4 J but just need to know how to get there.
What is the frequency of the photons emitted by hydrogen atoms when they undergo transitions from n=5 to n=3.
Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom?
How do you write chemical formulas for: cobalt (II) hydorgen carbonate and sulfur hexafluoride
A typical gauge pressure for optimal performance of automobile tires is 32 lb/in2. What is this pressure in grams per square centimeter and kilograms per square meter
Atoms and molecules consist of electrons and nuclei. When no bonds exist between atoms, electrons are on discrete energy levels called orbitals: those levels where electrons reside at zero degree Kelvin are called ground states
The solution gives an absorbance of 0.102 at 227nm using a 1.0 cm cell. A separate water sample containing benzene gives an absorbance of 0.0844 at 227nm in a 1.0 cm cell. What is the concentration of benzene in the water sample
When 0.538 g of Neon is added to an 800 cm^3 bulb containing a sample of argon, the total pressure of the gases is found to be 1.17 atm at a temperature of 295 K. Find the mass of the argon in the bulb.
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